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Topic 12: Atomic Structure
For HL students only
1. [1 mark]
Successive ionization energies of an element, X, are shown.
What energy, in kJ mol−1, is required for element X to reach its most stable oxidation state in ionic compounds?
A. 740
B. 1450
C. 2190
D. 7730
2a. [1 mark]
Consider the following reaction:
Cu2+ (aq) + Fe (s) → Fe2+ (aq) + Cu (s)
State the ground-state electron configuration for Fe2+.
2b. [1 mark]
The mass spectrum for copper is shown:
Show how a relative atomic mass of copper of 63.62 can be obtained from this mass spectrum.
2c. [1 mark]
Predict, with a reason, whether Cu or Cu2+ has the greater ionization energy.
2d. [2 marks]
Determine the frequency, in s−1, of a photon that will cause the first ionization of copper. Use sections 1, 2 and 8 of the data booklet.
2e. [2 marks]
Outline the magnetic properties of iron by referring to its electron configuration.
3. [1 mark]
The graph shows the first six ionization energies of an element.
In which group is the element?
A. 13
B. 14
C. 15
D. 16
4a. [1 mark]
Iron(II) disulfide, FeS2, has been mistaken for gold.
State the full electronic configuration of Fe2+.
4b. [2 marks]
Explain why there is a large increase from the 8th to the 9th ionization energy of iron.
4c. [1 mark]
Calculate the oxidation state of sulfur in iron(II) disulfide, FeS2.
4d. [1 mark]
Describe the bonding in iron, Fe (s).
5. [1 mark]
Which statement explains why the second ionization energy of aluminium is higher than the first ionization energy of magnesium?
A. Ionization energy increases along period 3.
B. 3p electrons are at a higher energy level than 3s electrons.
C. 3p electrons are further away from the nucleus than 2p electrons.
D. Both have the same number of electrons and aluminium has one more proton.
6a. [2 marks]
Electron transitions are related to trends in the periodic table.
Explain the general increase in trend in the first ionization energies of the period 3 elements, Na to Ar.
6b. [1 mark]
Sodium emits yellow light with a frequency of 5.09 × 1014 Hz when electrons transition from 3p to 3s orbitals.
Calculate the energy difference, in J, between these two orbitals using sections 1 and 2 of the data booklet.
7. [1 mark]
A period 3 element, M, forms an oxide of the type M2O. Which represents the first four successive ionization energies of M?
8a. [1 mark]
Magnesium is a group 2 metal which exists as a number of isotopes and forms many compounds.
Magnesium ions produce no emission or absorption lines in the visible region of the electromagnetic spectrum. Suggest why most magnesium compounds tested in a school laboratory show traces of yellow in the flame.
8b. [2 marks]
(i) Explain the convergence of lines in a hydrogen emission spectrum.
(ii) State what can be determined from the frequency of the convergence limit
If you need the markscheme, including the examiners' reports for each question, and more exam and teaching materials on this topic, contact me through the contact page